Quantum Numbers in Chemistry

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Questions and Answers

What does the principal quantum number (n) indicate?

  • The shape of the orbital
  • The size of an electron shell (correct)
  • The type of sub-shell
  • The energy of an electron

The azimuthal quantum number (l) can have values greater than or equal to 1.

False (B)

What shape is represented by l = 1?

dumbbell

The subshell corresponding to n = 3 and l = 0 is called the ______.

<p>3s</p> Signup and view all the answers

Match the quantum numbers with their corresponding subshells:

<p>1, 0 = 1s 2, 1 = 2p 3, 2 = 3d 4, 3 = 4f</p> Signup and view all the answers

What does the magnetic quantum number ($M_1$) describe?

<p>The orientation of an electron's orbital (B)</p> Signup and view all the answers

The values of the spin quantum number ($S$) are specifically numbered.

<p>False (B)</p> Signup and view all the answers

How many orbitals are present in the d sub-shell according to the magnetic quantum number ($M_1$)?

<p>5</p> Signup and view all the answers

The number of orbitals for the f sub-shell is ___.

<p>7</p> Signup and view all the answers

Match the sub-shells with the corresponding values of the magnetic quantum number ($M_1$):

<p>S = 0 P = -1, 0, +1 d = -2, -1, 0, +1, +2 f = -3, -2, -1, 0, +1, +2, +3</p> Signup and view all the answers

Flashcards

Principal Quantum Number (n)

Represents the electron shell's energy level and size. Larger 'n' means a larger and higher energy shell.

Azimuthal Quantum Number (l)

Determines the shape of an electron orbital within a shell.

Subshell

A specific energy level within a shell, determined by the principal quantum number (n) and the azimuthal quantum number (l).

Number of Subshells

The number of sub-shells within each shell is determined by the formula: n-1

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How does Orbital Shape relate to Chemical Properties?

The shape of an electron orbital determines the element's physical and chemical properties.

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Magnetic Quantum Number (ml)

The magnetic quantum number (ml) describes the orientation of an electron's orbital around the nucleus. It tells us how many orbitals of that particular shape exist within a subshell and how they are spatially oriented. Its values range from -l to +l, including 0. For example, a 'p' subshell (l=1) has three orbitals: ml = -1, 0, +1.

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Angular Momentum Quantum Number (l)

The angular momentum quantum number (l) describes the shape of an electron's orbital. It's determined by the number of subshells within an energy level. Each subshell has a characteristic shape and corresponds to a specific value of l: s (l=0), p (l=1), d (l=2), and f (l=3), with increasing complexity.

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Spin Quantum Number (s)

The spin quantum number (s) describes the intrinsic angular momentum, or spin, of an electron. It's analogous to an electron spinning on its axis, generating a magnetic field. It has two possible values: +1/2 (spin up) and -1/2 (spin down).

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How many orbitals in a subshell?

The number of possible values for the magnetic quantum number (ml) depends on the angular momentum quantum number (l). The number of possible ml values corresponds to the number of orbitals in a subshell.

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What are the possible values of the spin quantum number?

The spin quantum number (s) has two possible values: +1/2 (spin up) and -1/2 (spin down). This indicates the two possible orientations of the electron's spin.

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What could observations of straight lines, few particles, and empty space indicate?

The observations listed are possibly related to experiments where charged particles are emitted from a source. The straight lines suggest trajectories, and few particles indicate a specific event or a small probability of certain outcomes. The empty space could be an area affected or not affected by the released particles.

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